Explain why a σ bond formed by overlap of an s orbital with an sp 3 orbital of carbon is stronger than a σ bond formed by overlap of an s orbital with a p orbital of carbon.

Hey, everyone, let's do this problem and says the oxygen hydrogen bond in water is formed by the overlap of an S orbital with an SP three orbital. Why is this bond stronger than the bond that would be formed by the overlap of an S orbital with a P orbital? So let's draw the overlap of an S orbital with a P orbital. And then we'll compare that to the oxygen hydrogen bond mentioned in the problem. So drawing an S orbital, we know that has a spherical shape in a P orbital has this sideways, double lobe shape With two different phases. Alright. And then drawing an S orbital with an sp three orbital, which where does that come from? Let's draw water really quick. So we have oxygen with two hydrogen ins that oxygen has two lone pairs. So we see that we know hydrogen has an S orbital only and this oxygen has 1234 charge centers, which is why it is S P three hybridized. So drawing again the S orbital our sphere, but now the sp three hybridized orbital is going to have two lobes like the P orbital. But since we have the hybridization of four orbital's, the S and three P orbital's that lobe, one lobe is going to be much larger due to higher electron density. So the SP three is going to have a larger lobe than the P orbital, which has a smaller lobe. And that means it's going to have a higher electron density, the sp three orbital compared to that in hybridized P orbital. So when the S orbital is overlapped with an sp three orbital, the magnitude of that overlap is much stronger than the overlap between the S and the un hybridized P orbital. Therefore, the bond formed by the overlap of an S and SP three orbital is going to be stronger than that bond that is formed by the overlap of an S and P orbital. So the correct answer for this problem is the large lobe of the sp three orbital has a greater electron density compared to the P orbital. Therefore, the sp three orbital overlaps more strongly with an S orbital. And that makes a, the correct answer for this problem. That's it for this one. I hope this video is helpful and thanks for watching.

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Hybridization

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1. A Review of General Chemistry

Hybridization

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Problem 28

Textbook Question

Explain why a σ bond formed by overlap of an s orbital with an sp³ orbital of carbon is stronger than a σ bond formed by overlap of an s orbital with a p orbital of carbon.

Verified step by step guidance

Understand the nature of the orbitals involved: An s orbital is spherical and has a high electron density near the nucleus. An sp³ orbital is a hybrid orbital formed by mixing one s orbital and three p orbitals, resulting in a shape that is more directional and has significant electron density along the bonding axis. A p orbital, on the other hand, is dumbbell-shaped and less directional compared to an sp³ orbital.

Consider the concept of orbital overlap: The strength of a σ bond depends on the extent of overlap between the orbitals of the two atoms. Greater overlap leads to a stronger bond because it allows for more effective sharing of electrons between the nuclei.

Compare the overlap of s and sp³ orbitals: The sp³ orbital has a larger lobe pointing in a specific direction, which allows for better overlap with the spherical s orbital. This directional nature of the sp³ orbital maximizes the electron density in the bonding region, leading to a stronger bond.

Compare the overlap of s and p orbitals: The p orbital is less directional and has a smaller region of electron density along the bonding axis compared to the sp³ orbital. This results in less effective overlap with the s orbital, making the σ bond weaker.

Conclude the reasoning: The σ bond formed by the overlap of an s orbital with an sp³ orbital is stronger than that formed with a p orbital because the sp³ orbital's directional nature and larger lobe allow for greater overlap and more effective electron sharing in the bonding region.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Orbital Hybridization

Orbital hybridization is the process by which atomic orbitals mix to form new hybrid orbitals that are degenerate in energy. In carbon, the sp3 hybridization involves the mixing of one s orbital and three p orbitals, resulting in four equivalent sp3 orbitals. This hybridization allows for stronger sigma bonds due to the optimal overlap of orbitals in bonding.

Sigma (σ) Bonds

Sigma bonds are the strongest type of covalent bond formed by the head-on overlap of atomic orbitals. The strength of a σ bond is influenced by the extent of overlap between the orbitals involved. The overlap of an sp3 hybrid orbital with an s orbital is more effective than that of a p orbital with an s orbital, leading to a stronger σ bond.

Orbital Overlap

Orbital overlap refers to the region where two atomic orbitals come into contact, allowing for the sharing of electrons. The greater the overlap, the stronger the bond formed. In the case of an sp3 and s orbital overlap, the geometry and orientation of the hybrid orbitals facilitate a larger area of overlap compared to the overlap between an s and a p orbital, resulting in a stronger bond.

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